Chemistry Unit 14 Acids and Bases

Ionizable

Acids vary in the number of hydrogen atoms they have that can form hydrogen ions

Very electronegative elements

Only type of elements bonded with hydrogen ions are ionizable

dissociation

very polar bonds that release hydrogen ions when dissolved in water

dissociation of hydrochloric acid

HCI→ H⁺ + Cl⁻

dissociation of hydrochloric acid in water

HCI + H2O → Cl⁻ + H3O⁺

Hydronium or Oxonium

forms when a water molecule gains a hydrogen ion

Characteristics of Acids

• have a sour taste (citric acid in lemons)

• have a low PH: turns litmus paper red

• react strongly with metals, carbonates and bases

Characteristics of Bases

• Have a bitter taste

• have a slippery feel

• high PH: turns litmus paper blue

• reacts with fat, oil, acids

Arrhenius Acids

hydrogen-containing compounds that dissociate/ionize to yield hydrogen (H+) or hydronium (H3O⁺) ions in aqueous solutions.

Arrhenius Bases

hydroxide-containing compounds that dissociate to yield hydroxide (OH-) ions in aqueous solutions.

Aqueous solutions of acids and bases

strong or weak electrolytes

Arrhenius Acid classification

Monoprotic, diprotic, and triprotic

• based on the number of hydrogen atoms that are ioinizable

• a strong acid is a strong electrolyte

• a weak acid is a weak electrolyte

What do Arrhenius Bases produce when they dissociate

produces a metal ion or a cation, along with a hydroxide ion

Bronstead-Lowry Acid

an acid that is a hydrogen ion donor

Bronstead-Lowry Base

a base that is a hydrogen ion acceptor

Amphoteric

substances that can be both acid and base

• water is amphoteric

conjugate acid

ion or molecule formed when it gains a hydrogen ion

conjugate base

ion or molecule formed after an acid loses a hydrogen ion

pH

a value that expresses the acidity or basicity of a solution

pOH

the measure of hydroxide ion concentration of a solution